Find the gram-molecular mass of the gas if the density of a diatomic gas at STP is $1.43$ grams $/$ liter.

14.3

No worries! We‘ve got your back. Try BYJU‘S free classes today!

32.0

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

48.0

No worries! We‘ve got your back. Try BYJU‘S free classes today!

64.3

No worries! We‘ve got your back. Try BYJU‘S free classes today!

224

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B $32.0$ g
1 mole of a gas at STP occupies a volume of 22.4 L.
The density of the gas at STP is 1.43 g/L.
The mass of 22.4 L of gas is $1.43 g / L \times 22.4 = 32.0 g$ .
Mass of 1 mole of the gas is equal to the gram-molecular mass of the gas.
Hence, gram-molecular mass of the gas is 32.0 g.

Suggest Corrections

Similar questions

80

1.43 g L^{- 1}

2 H_{2} O (I) - 2 H_{2} (g) + O_{2} (g)

Join BYJU'S Learning Program